Preparation of Ag0 Nanoparticles by EDM Method as Catalysts for Oxygen Reduction

At present, platinum-based catalysts are the best cathode catalysts, but due to their high prices, they are difficult to use widely. Under alkaline conditions, silver is a better low-cost substitute. Here, a physical preparation method—electrical discharge machining (EDM)—is used to prepare Ag0 nanoparticles. The method is simple and has a high yield. The diameter of prepared nanoparticles is about 30 nm and the nanoparticle surface is rich in defects. These defects enhance the adsorption of O2. In addition, defects can cause tensile strain on the silver catalyst, causing the d-band center of silver to move upward. The defects and the upward shift of the d-band center jointly improve the adsorption energy and catalytic performance of Ag0. This work provides a new method for the engineering construction of surface defects and the preparation of metal catalysts.


Introduction
The rapid growth of global demand for energy and the massive consumption of traditional fossil fuels are driving people to seek new sources of clean energy. Among these, high energy density fuel cells are an advanced energy storage and conversion device for meeting the requirements of environmentally sustainable energy [1,2]. However, the power of the fuel cell stack is often affected by the slow kinetics of the cathode oxygen reduction reaction (ORR), resulting in an energy conversion efficiency far from the thermodynamic ideal [3]. Platinum-based catalysts are one of the most efficient ORR catalysts yet discovered, and can effectively reduce the energy barrier and greatly improve the conversion efficiency. However, due to their high cost and scarcity, large-scale commercial application remains a huge challenge. It is necessary to search for non-platinum-based catalysts with excellent catalytic performance. Low-priced metal oxides [4,5], nitrides [6,7], sulfides [8,9] and silver-based catalysts [10][11][12] have broad prospects. Among them, silver-based catalysts have shown good ORR activity under alkaline conditions [13]. Moreover, silver has good electrical conductivity and its price is about a fiftieth of the price of platinum [14], which makes silver an attractive low-cost alternative. However, the adsorption capacity of silver for O 2 is weak, and the catalytic activity of silver is not as excellent as that of platinum, so the adjustment of silver's properties is necessary.
The strain effect is an effective strategy to improve catalyst activity [15]. For a transition metal with more than half of the d-band filled, under tensile strain, the center of the d-band moves upward relative to the Fermi level, resulting in a decrease in the occupancy rate of the antibonding states below the Fermi level, thus increasing the adsorption energy of the intermediate reaction [16][17][18]. For example, cobalt (II) oxide, an inactive HER material, changes the adsorption energy of hydrogen by introducing a tensile strain on the surface, allowing it to be converted to a highly efficient electrocatalyst toward HER [19]. Because of the low adsorption energy of silver for O 2 , the tensile strain effect can be introduced to regulate the adsorption energy of a silver catalyst. 2 of 9 Structural defects can cause local microstrains on the surface of the catalyst [20][21][22]. In addition, surface defects are also one of the important factors affecting the adsorption energy of catalysts, and many results have confirmed that defects on the catalyst surface positively affect the electrochemical reaction [23,24]. Defects in the catalyst can alter the electron density and charge distribution of the catalyst and increase the adsorption of reaction intermediates. Therefore, building strain through surface defects is a feasible method. Lin Guo [25] reported that the quenching effect can change the catalyst surface structure, and that the surface of metal oxide nanocatalysts could be adjusted by rapidly cooling them in a salt solution, which resulted in a large number of defects on the quenched nanocatalyst surface. Xiwen Du [26] reported the preparation of defect-rich metallic silver by laser ablation for the hydrogen evolution reaction. However, these surface-engineering strategies, while enabling the development of better catalysts, are difficult for large-scale commercial applications due to low production, long preparation cycles, and expensive equipment. Therefore, it is necessary to develop a general strategy that is simple, low cost, and capable of mass production.
Here, we adopt a physical method-electrical discharge machining (EDM). The method is carried out in liquid at room temperature. After discharging, the electric field between the electrodes begins to increase, and when the electric field strength is greater than the dielectric strength of the dielectric, the electric field force causes the cathode to emit electrons. Electrons emitted from the cathode rapidly collide with neutral atoms at the anode, resulting in the shedding of outer electrons and the generation of cations that flow rapidly to the negative electrode, forming a high-temperature ion channel [27]. When the plasma reaches the silver surface, the silver surface melts and evaporates, which is then rapidly cooled and quenched under room-temperature liquid to form defect-rich Ag 0 nanoparticles. The method is simple and makes it easier to produce Ag 0 nanoparticles. The most important aspect of it is that this method has a short cycle and can be prepared on a large scale, which solves the chemical method's problem of insufficient yields. This strategy provides an economical and efficient way to prepare metal nanoparticles and makes it possible for non-noble metals to replace commercial platinum carbon catalysts in alkaline or acidic fuel cells.
NPS-Ag 0 was prepared in an EDM machine (Shanghai Zhantie Precision Machinery Co., Ltd., Shanghai, China), model AF-1100. Firstly, a silver electrode was fixed in the center of the conductive iron container. The container was connected with the negative electrode of the AF-1100 EDM, and the other silver electrode was connected with the servo system as the anode. Subsequently, 500 mL of deionized water was poured into the container as coolant. The distance between the two silver electrodes was adjusted by a servo system so that the two electrodes immersed in the deionized water could generate electrical sparks through discharge. Due to the extremely short discharge time and area, the energy in the discharge area was concentrated; the temperature in the discharge area was as high as 10,000 degrees Celsius. The silver on the surface was then fused into silver vapor or silver droplets at high temperature with an electric spark. These molten silver droplets cooled rapidly when they encountered water to form silver nanoparticles, which were then collected by centrifugation. X-ray diffraction (XRD) with a Rigaku D8/Max 2500PC (Rigaku Science Co., Tokyo, Japan) was used to analyze the crystal structure of this phase. The scanning speed of 2θ was 10-90 • , and the test voltage was 40 kV. A scanning electron microscope (SEM) S-4800 made by the Hitachi Company (Tokyo, Japan) was used for the morphological analysis of samples. The microstructure of the material was analyzed by transmission electron microscopy (TEM, FEI Corporation, OR, USA) (acceleration voltage of 200 V). The valence states and valence band spectra of the elements were measured with X-ray photoelectron spectroscopy (XPS, Thermo Fisher Scientific, Waltham, MA, USA) of Perkin Elmer Phi1600.
A quantity of 1.0 mg NPS-Ag 0 and 1.5 mg carbon was dispersed in 200 µL deionized water and 200 µL isopropyl alcohol for 30 min by ultrasound to mix the electrode ink evenly. Subsequently, 12 µL Nafion was added for further ultrasound for 30 min. A Nafion solution as a catalyst coating can effectively reduce the transmission resistance of the substance and the resistance of the electrode. This preparation method of Ag is consistent with that of NPS-Ag 0 . 5 mg 20 wt% Pt/C catalyst were dispersed in 500 µL deionized water and 500 µL isopropanol for 30 min by ultrasound, and 30 µL Nafion was added for further ultrasound for 30 min. The electrochemical test was carried out in a three-electrode cell at room temperature, with a reference electrode saturated calomel (Hg/HgO) and counter electrode platinum wire (Pt). The test was carried out in an electrochemical workstation of type CHI760E. Before the test, 0.1 M KOH solution was permeated with O 2 for 30 min to saturate it. A quantity of 5.6 µL of catalyst was dropped into the glassy carbon disk of the polished rotating disk electrode (RDE) (0.07065 cm 2 ). The cyclic voltammetry curve (CV) was measured in a KOH solution saturated with O 2 at a sweep rate of 50 mV s −1 , and the number of cycles was 20; that is, until the curve became stable. The scanning voltammetry curve (LSV) (1600 rpm) was measured in O 2 -saturated KOH solution at a sweep rate of 5 mV s −1 in the range of 0-1.2 V (vs. RHE).
Calculations: The electron transfer number of oxygen reduction calculated as follows: where i represents the measured electricity density, i k is the dinetic density, and i d is the diffusion-limited current density. Besides this, n, F, A, C 0 , D O2 , v, and w are the number of electrons transferred, the Faraday constant (96,485 C mol −1 ), the electrode geometry surface area, the concentration of oxygen in the 0.1 M KOH electrolyte (C 0 = 1.26 × 10 −6 mol cm −3 ), the diffusion coefficient (1.9 × 10 5 cm 2 ·s −1 ), the solution viscosity (v = 0.01 cm 2 ·s −1 ) and the rotating angular velocity of the electrode (rad·s −1 ), respectively. Figure 1 shows the synthesis process of silver nanoparticles prepared by the electric spark method. As shown in the figure, after electrification, an electric spark is generated between the two electrodes, and then the surface of the silver electrode is melted and evaporated by a high temperature electric spark. Under the cooling action of deionized water, the silver vapor gradually agglomerates and then nucleates. Then the silver vapor adheres to the nucleus and the atom grows gradually to form silver nanoparticles. The quenching effect of high temperature silver vapor in deionized water makes silver nanoparticles rich in vacancies and other point defects, while Ag has the lowest stacking fault energy (16 mJm −2 ) among all elemental metals, and when the number of vacancies reaches a certain amount, the atomic surface collapses very easily and thus forms a stacking fault.  By scanning/transmission electron microscopy (SEM/TEM) characterization, further understanding of the structure and morphology of the NPS-Ag 0 was reached. As shown in Figure 3a,d., due to the energy of electrical discharge, particles of different sizes were inevitably generated in the processed products (Figure 3a). Except for some large particles with a diameter of 200 nm, most particles were around 30 nm. The product was classified by a high-speed centrifuge at different rotating speeds. The NPs-Ag 0 obtained was in the shape of a particle with a diameter of about 30 ± 12 nm (Figure 3b). NPS-Ag 0 high-resolution TEM images show the structural defects of the new material (Figure 3c,d). Figure 3c shows the stacking fault of the new material. Under the quenching effect of deionized water, the high temperature silver steam produced vacancies, dislocation, and other defects. A large number of vacancies clump together, causing the silver (111) crystal plane to collapse, forming a stacking fault [26,28]. Additionally, the amorphous region and twin  By scanning/transmission electron microscopy (SEM/TEM) characterization, further understanding of the structure and morphology of the NPS-Ag 0 was reached. As shown in Figure 3a,d., due to the energy of electrical discharge, particles of different sizes were inevitably generated in the processed products (Figure 3a). Except for some large particles with a diameter of 200 nm, most particles were around 30 nm. The product was classified by a high-speed centrifuge at different rotating speeds. The NPs-Ag 0 obtained was in the shape of a particle with a diameter of about 30 ± 12 nm (Figure 3b). NPS-Ag 0 high-resolution TEM images show the structural defects of the new material (Figure 3c,d). Figure 3c shows the stacking fault of the new material. Under the quenching effect of deionized water, the high temperature silver steam produced vacancies, dislocation, and other defects. A large number of vacancies clump together, causing the silver (111) crystal plane to collapse, forming a stacking fault [26,28]. Additionally, the amorphous region and twin By scanning/transmission electron microscopy (SEM/TEM) characterization, further understanding of the structure and morphology of the NPS-Ag 0 was reached. As shown in Figure 3a-d, due to the energy of electrical discharge, particles of different sizes were inevitably generated in the processed products (Figure 3a). Except for some large particles with a diameter of 200 nm, most particles were around 30 nm. The product was classified by a high-speed centrifuge at different rotating speeds. The NPs-Ag 0 obtained was in the shape of a particle with a diameter of about 30 ± 12 nm (Figure 3b). NPS-Ag 0 highresolution TEM images show the structural defects of the new material (Figure 3c,d). Figure 3c shows the stacking fault of the new material. Under the quenching effect of deionized water, the high temperature silver steam produced vacancies, dislocation, and other defects. A large number of vacancies clump together, causing the silver (111) crystal plane to collapse, forming a stacking fault [26,28]. Additionally, the amorphous region and twin defects were observed in the high-resolution transmission electron microscope ( Figure 3d). These defects increase the active sites of NPS-Ag 0 , allowing O 2 to adsorb better and diffuse to an adjacent plane where the intermediate is formed, which is easily released due to its relatively weak binding [14,29]. On the other hand, these structural defects induce tensile strain of the catalyst and regulate the electronic structure of NPS-Ag 0 , leading to drastic changes in the interaction between NPS-Ag 0 and intermediates [30]. These factors enhance the ORR activity. However, there is no obvious defect on the surface of Ag nanoparticles ( Figure S1). In addition, The typical lattice stripes consistent with the (111) face lattice of the cubic silver phase were revealed by measuring the lattice stripe spacing of NPS-Ag 0 and Ag with a spacing of 0.243 nm for NPS-Ag 0 , which is increased compared to 0.236 nm for Ag ( Figure S2), further confirming the tensile strain of NPS-Ag 0 .

Synthesis and Characterization
Metals 2021, 11, x FOR PEER REVIEW 5 of 9 defects were observed in the high-resolution transmission electron microscope (Figure 3d). These defects increase the active sites of NPS-Ag 0 , allowing O2 to adsorb better and diffuse to an adjacent plane where the intermediate is formed, which is easily released due to its relatively weak binding [14,29]. On the other hand, these structural defects induce tensile strain of the catalyst and regulate the electronic structure of NPS-Ag 0 , leading to drastic changes in the interaction between NPS-Ag 0 and intermediates [30]. These factors enhance the ORR activity. However, there is no obvious defect on the surface of Ag nanoparticles ( Figure S1). In addition, The typical lattice stripes consistent with the (111) face lattice of the cubic silver phase were revealed by measuring the lattice stripe spacing of NPS-Ag 0 and Ag with a spacing of 0.243 nm for NPS-Ag 0 , which is increased compared to 0.236 nm for Ag ( Figure S2), further confirming the tensile strain of NPS-Ag 0 .

Electrochemical Measurements
The ORR catalytic performance of NPS-Ag 0 catalyst was evaluated by rotating disk electrode (RDE) in 0.1 M potassium hydroxide and compared with that of C, Ag, and 20% Pt/C. First, different catalysts were characterized by cyclic voltammetry (CV) ( Figure S3). Compared with a N2 saturated solution, the CV of different catalysts showed a definite oxygen reduction peak in the O2-saturated solution, and the reduction peak potential of NPS-Ag 0 was higher than that of Ag, which confirmed the excellent oxygen reduction of NPS-Ag 0 . The linear sweep voltammetry (LSV) curves of all catalysts are shown in Figure  4a. The onset potential was 1% of the limiting current density [10,31]. This onset potential reflects the overpotential of the catalyst. The onset potential (E0) of NPS-Ag 0 was close to 0.943 V, while Ag and Pt/C were 0.912 V and 0.989 V, respectively ( Figure S4). The higher the starting potential is, the lower the overpotential. This indicates a higher catalytic activity. In addition, near the half-wave potential the kinetics of the catalyst are reflected. The half-wave potential (E1/2) of NPS-Ag 0 (0.8 V) was slightly lower than that of Pt/C (0.85 V), and had better performance than that of Ag (0.74 V). The increase in ORR activity indicates that the adsorption of NPS-Ag 0 on the intermediate was improved.
In an alkaline medium, the cathode oxygen reduction reaction can be carried out along a two electron pathway or a four electron pathway. The electron transfer number of the catalyst can be calculated and evaluated by the Koutecky-Levich (K-L) equation. The ORR polarization curves of the catalyst were measured at different rotating speeds (Figure

Electrochemical Measurements
The ORR catalytic performance of NPS-Ag 0 catalyst was evaluated by rotating disk electrode (RDE) in 0.1 M potassium hydroxide and compared with that of C, Ag, and 20% Pt/C. First, different catalysts were characterized by cyclic voltammetry (CV) ( Figure S3). Compared with a N 2 saturated solution, the CV of different catalysts showed a definite oxygen reduction peak in the O 2 -saturated solution, and the reduction peak potential of NPS-Ag 0 was higher than that of Ag, which confirmed the excellent oxygen reduction of NPS-Ag 0 . The linear sweep voltammetry (LSV) curves of all catalysts are shown in Figure 4a. The onset potential was 1% of the limiting current density [10,31]. This onset potential reflects the overpotential of the catalyst. The onset potential (E 0 ) of NPS-Ag 0 was close to 0.943 V, while Ag and Pt/C were 0.912 V and 0.989 V, respectively ( Figure S4). The higher the starting potential is, the lower the overpotential. This indicates a higher catalytic activity. In addition, near the half-wave potential the kinetics of the catalyst are reflected. The half-wave potential (E 1/2 ) of NPS-Ag 0 (0.8 V) was slightly lower than that of Pt/C (0.85 V), and had better performance than that of Ag (0.74 V). The increase in ORR activity indicates that the adsorption of NPS-Ag 0 on the intermediate was improved. rent and ECSA, as shown in Figure 4d. At 0.85 V, the mass activity of NPS-Ag 0 was 6.52 mA·mg −2 , which was 221% higher than that of Ag (2.95 mA mg −2 ). The specific activity of NPS-Ag 0 was 0.079 mA·cm −2 . It is higher than 0.047 mA cm −2 of Ag .The particle size of NPS-Ag 0 was similar to that of Ag, but the mass activity and specific activity of NPS-Ag 0 increased greatly, which indicated that the defect and tensile strain significantly improved the oxygen reduction efficiency of NPS-Ag 0 .  In an alkaline medium, the cathode oxygen reduction reaction can be carried out along a two electron pathway or a four electron pathway. The electron transfer number of the catalyst can be calculated and evaluated by the Koutecky-Levich (K-L) equation. The ORR polarization curves of the catalyst were measured at different rotating speeds ( Figure S5) and the linear behavior of the inverse current with the inverse of the square root of rotation speed is presented in Figure 4b. According to the calculation of the K-L slope, the ORR of NPS-Ag 0 at 0.5 V mainly involves the four-electron transfer process, indicating that there is a major four-electron transfer pathway for NPS-Ag 0 in 0.1 M potassium hydroxide solution, and O 2 is completely reduced to OH-. The ORR kinetic process can be reflected in the Tafel diagram shown in Figure 4c.The Tafel slope of NPS-Ag 0 is 105 mV·dec −1 , less than Ag (120 mV·dec −1 ). It is obvious that NPs-Ag 0 has a better kinetic process than Ag. It is shown that the defects can greatly improve the kinetics of NPS-Ag 0 and enhance the electrical conductivity so that the electrons can be transferred quickly. The good electrocatalytic performance of the NPS-Ag 0 catalyst for ORR was partly attributed to the defects on the surface of the catalyst, which changed the electron density and charge distribution of NPS-Ag 0 and increased the number of active sites. In the other part, due to tensile strain, the center of d-band moved upward, which enhanced the adsorption energy of intermediate products. These two aspects reduced the overpotential of NPS-Ag 0 and significantly increased the catalyst activity.
In addition, the intrinsic catalytic activity of the catalyst was characterized by electrochemical active surface area (ECSA), mass activity (J k, Mass ), and the specific activity (J k, Specific ) of the catalyst. First, the ECSA of the silver-based catalyst was measured by the Pb underpotential deposition method. Under the voltage of 0.25 vs. RHE, 300 s of Pb was deposited. In general, the theoretical value of Pb deposition on the silver surface is 260 uC·cm −2 [10]. Figure S6 shows the normalized ECSA graph. The ECSA of NPS-Ag 0 was greater than that of Ag, indicating that the defects in the catalyst increased the active site of NPS-Ag 0 . Figure 4 shows the mass activity and specific activity of the catalyst.
The mass activity and specific activity of the catalyst were calculated by kinetic current and ECSA, as shown in Figure 4d. At 0.85 V, the mass activity of NPS-Ag 0 was 6.52 mA·mg −2 , which was 221% higher than that of Ag (2.95 mA mg −2 ). The specific activity of NPS-Ag 0 was 0.079 mA·cm −2 . It is higher than 0.047 mA cm −2 of Ag. The particle size of NPS-Ag 0 was similar to that of Ag, but the mass activity and specific activity of NPS-Ag 0 increased greatly, which indicated that the defect and tensile strain significantly improved the oxygen reduction efficiency of NPS-Ag 0 .
The long-term stability of catalysts is also important in practical applications. The chronometric current method is a common method to measure the stability of a catalyst. The long-term stability of NPS-Ag 0 , Ag, and Pt/C was measured at a constant voltage of 0.5 V (vs. RHE) in a 0.1M KOH solution, as shown in Figure 5. The current of NPS-Ag 0 can still reach 91% of the initial current after 30,000 s, while the current of Ag and Pt/C can only reach 88% and 73% of the initial current at the same time and electrolyte solution, respectively. Activity and long-term stability studies show that NPS-Ag 0 materials can be used as high-efficiency electrocatalysts for ORR. Tafel plots from catalysts. (d) Comparison of catalytic activities for ORR of each sample given as the jk,mass and jk,specific.
The long-term stability of catalysts is also important in practical applications. The chronometric current method is a common method to measure the stability of a catalyst. The long-term stability of NPS-Ag 0 , Ag, and Pt/C was measured at a constant voltage of 0.5 V (vs. RHE) in a 0.1M KOH solution, as shown in Figure 5. The current of NPS-Ag 0 can still reach 91% of the initial current after 30,000 s, while the current of Ag and Pt/C can only reach 88% and 75% of the initial current at the same time and electrolyte solution, respectively. Activity and long-term stability studies show that NPS-Ag 0 materials can be used as high-efficiency electrocatalysts for ORR.

The d-Band Center of NPS-Ag 0 and Ag
In order to further understand the electronic structure and electronic perturbation of the silver-based catalyst, X-ray photoelectron spectroscopy (XPS) and valence band spectroscopy (VBS) measurements were performed. This is shown in Figure 6a-b. Two peaks of NPS-Ag 0 were observed at 368.2 eV (Ag 3d3/2) and 374.2 eV (Ag 3d5/2), corresponding to metal Ag0, indicating that no silver oxide was produced. Two Ag peaks were observed at 368.4 eV (Ag 3d3/2) and 374.4 eV (Ag 3d5/2), and the NPS-Ag 0 peak was negatively offset by 0.2 eV from Ag, which confirmed that the electron density of NPS-Ag 0 was increased compared with Ag (d-band center shifted upward) [14]. In addition, the valence band spectra of NPS-Ag 0 and NPS-Ag 0 were tested by XPS. The d-band centers of NPS-Ag 0 and Ag are shown in Figure 6c. The experimental results show that the surface electronic structure of NPS-Ag 0 is significantly different from that of Ag. The d-band center of NPS-Ag 0 is 5.95 eV, and the inherent d-band center of Ag is 6.45 eV, as calculated by the valence band spectrum. The d-band center of NPS-Ag 0 is higher than the relative Fermi level of Ag. Different metals have different adsorption energies for intermediates. J. K. Nørskov [32] and others established a volcano map based on the calculation of the adsorption energies of various metals on intermediates. According to the volcanic map of oxygen adsorption, Ag has a weak adsorption on O2, so it is necessary to raise the center of the d-band by tensile strain. In general, due to the upward shift of the d-band center, the adsorption of NPS-Ag 0 for intermediates is enhanced, thus enhancing the ORR performance of NPS-Ag 0 .

The d-Band Center of NPS-Ag 0 and Ag
In order to further understand the electronic structure and electronic perturbation of the silver-based catalyst, X-ray photoelectron spectroscopy (XPS) and valence band spectroscopy (VBS) measurements were performed. This is shown in Figure 6a-b. Two peaks of NPS-Ag 0 were observed at 368.2 eV (Ag 3d 3/2 ) and 374.2 eV (Ag 3d 5/2 ), corresponding to metal Ag 0 , indicating that no silver oxide was produced. Two Ag peaks were observed at 368.4 eV (Ag 3d 3/2 ) and 374.4 eV (Ag 3d 5/2 ), and the NPS-Ag 0 peak was negatively offset by 0.2 eV from Ag, which confirmed that the electron density of NPS-Ag 0 was increased compared with Ag (d-band center shifted upward) [14]. In addition, the valence band spectra of NPS-Ag 0 and Ag were tested by XPS. The d-band centers of NPS-Ag 0 and Ag are shown in Figure 6c. The experimental results show that the surface electronic structure of NPS-Ag 0 is significantly different from that of Ag. The d-band center of NPS-Ag 0 is 5.84 eV, and the inherent d-band center of Ag is 6.27 eV, as calculated by the valence band spectrum. The d-band center of NPS-Ag 0 is higher than the relative Fermi level of Ag. Different metals have different adsorption energies for intermediates. J. K. Nørskov [32] and others established a volcano map based on the calculation of the adsorption energies of various metals on intermediates. According to the volcanic map of oxygen adsorption, Ag has a weak adsorption on O 2 , so it is necessary to raise the center of the d-band by tensile strain. In general, due to the upward shift of the d-band center, the adsorption of NPS-Ag 0 for intermediates is enhanced, thus enhancing the ORR performance of NPS-Ag 0 .

Conclusions
Silver nanoparticles were successfully prepared by EDM. The quenching effect led to the silver containing a large number of defects, which caused tensile strain in the silver nanoparticles. The defects and tensile strain enhanced the ORR activity of the silver nanoparticles. The silver nanoparticles prepared by this method have excellent properties, and the method is simple, its time cycle is short, and the silver nanoparticles can achieve mass production. As well as EDM's advantages of simplicity and high yield, it is also possible, by changing the electrode material or coolant, to prepare silver-based alloy catalysts or even other metals and alloy catalysts using this method.